d) Ka for HF = 6.6 * 10^(-4)
pH = pKa + log(F-/HF) = (4 - log(6.6)) + log(2) = 3.48
e) Since it has more number of F- ions, hence it will have more buffer capacity for addition of acids, which will react with the present F- ions in solution.
f) H2SO4 is a strong acid. Hence ideally it will give 2 moles of H+ per mole of H2SO4. But the leaving of second H+ is not that fast. Hence the [H+] will be more than 1 but less than 2 times. Hence the correct answer will be "Between 0.2 and 0.4M"
g)Since Ka for HNO2 is higher, hence it will be stronger acid, so it will lead to have lesser pH value. Hence the pH value will be higher for HClO
h) The Ksp expressio for mercury sulfate will be
Note - Post any doubts/queries in comments section.
d. (4 pts) Determine the pH of a buffer containing 0.10 M HF and 0.20 M...
What is the pH of a buffer solution containing 0.13 M HF and 5.0×10−2 M NaF? What is the pH of a buffer solution containing 1.0×10−2 M HF and 0.16 M NaF? Using the table given below for Ka values, compare the pH of an HF buffer that contains 0.13 MHF and 5.0x10-2 M NaF with another HF buffer that contains 1.0x10-2 MHF and 0.16 M NaF. Ka and K b values for selected weak acids and bases HF Acid...
what is the pH of a buffer solution containing 0.23 M HNO2 and 0.15 M NO2 Nitrous acid has a Ke of 4.5 x 10-4. Part A What is the pH of a buffer solution containing 0.23 M HNO2 and 0.15 M NO? Express your answer using two decimal places. 19 AEO ? pH = Submit Request Answer Provide Feedback Google Drive @ Quinet C Chego Coinmame R PL Access SIUE CHW11 Chapter 11 Homework Problem 25 25 of 25...
pH of buffer is calculated by the equation: pH=pK, +log (base/acid). Where pK= -log Kg. For nitrous acid HONO2 Kg = 4.0.10-4; for ammonia Kg = 5.6•10-10 Determine, whether the following solution is a buffer, if yes - calculate pH for the solution, which is prepared by mixing of: 0.2 L of 0.6 M HNO2 +0.4 L 0.1 M NH3 3.00 8.77 8.67 3.10
1. Rank the solutions in order of decreasing [H3O+]: 0.10 M HF, 0.10 M HCl, 0.10 M HClO, 0.10 M HC6H5O. 2. The beaker will be filled to the 0.50 L mark with a neutral solution. Set the pH to 3.95 by using the green arrows adjacent to the pH value indicated on the probe in the solution. Once you adjust the pH, note the corresponding OH− ion concentration in M as given in the graphic on the left side...
A 15 L buffer solution is 0.250 Min HF and 250 M in Ne Calculate the pH of the solution after the addition of 0.0500 moles of sold NOH. Assume no volume change upon the addition of base. The K, for HF 35 x 104 351 3.54 3.46 3.63 Which of the following is TRUE? An effective buffer has a [base)(acid] ratio in the range of 10 -100. A buffer can not be destroyed by adding too much strong base....
1) How would you make 300 ml of a 0.1 M sodium phosphate buffer, pH 7.0 (pKa = 7.2) phosphate dibasic (the conjugate base). 2) What are the concentrations of acetate and acetic acid in a 0.2 M acetate buffer pH 5.3? The pKa for acetic acid is 4.76. 3)You have 100 ml of 0.1 M acetate buffer pH 5.2 (pKa 4.76). You add 10 ml of 0.1 M NaOH. Calculate the resulting change in pH and the buffering capacity...
Question 1 1 pts Consider a solution that is 0.1 M HF and 0.1 M NaF. This is a mixture of conjugates in equal proportions, which tells you that it is a buffer. What two reactions are relevant to the pH in this situation? NaF --> Nat + F F+H2O <--> HF + OH- HF + NaF --> H+ +Na+ + F2 HF <--> H+ +F Ht+F<--> Nat + F" Question 2 1 pts A buffer solution contains a mixture...
1. A buffer is 0.100 M in HF and 0.100 M in NaF. When a small amount of nitric acid is added the pH only slightly drops. Write the chemical equation that shows the added nitric acid being neutralized by this buffer. 2. What is the pH of a buffer that is 0.120 M formic acid (HCHO2) and 0.080 M in potassium formate (KCHO2)? The Ka of formic acid is 1.8 x 10^ -4 . 3. The curve shows the...
2. (5 pts) A researcher wants to make a buffer of pH 4.60 using nitrous acid (K = 4.0 x 10-4) and sodium nitrite. a) Determine the approximate ratio of the two buffer components that she should use to get the desired pH. b) Evaluate the researcher's decision to use the nitrous acid/nitrite buffering system.
A buffer solution that is 0.10 M sodium acetate and 0.20 M acetic acid is prepared. Calculate the initial pH of this solution The K, for CH3COOH is 1.8 x 10-5 M. As usual, report pH to 2 decimal places. Answer: A buffered solution resists a change in pH. Calculate the pH when 21.2 mL of 0.031 M HCl is added to 100.0 mL of the above buffer. Answer: